Periodic Trends

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Trends on the periodic table

23 Terms

1

atomic radius

half the distance between the nuclei of two adjacent atoms of the same element

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2

atomic radius: down a group

radius increases - more energy levels create a larger radius

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3

atomic radius: across a period

radius decreases - there are more protons and no new energy levels (Zeffective is greater) so the radius shrinks

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4

shielding effect

decrease in the attraction of the valence electrons towards the protons due to the presence of the energy levels between the nucleus and valence electrons

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5

effective nuclear charge

the perceived attraction the electron has for the protons in the nucleus; the more shells there are, the weaker the Zeffective becomes b/c the protons are attracted to the electrons closest to the nucleus

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6

Ionization energy

amount of energy required to remove one valence electron form an atom and form a +1 ion

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7

ionization energy: down a group

energy decreases - Zeff is weaker due to more shielding, so the electrons require less energy to remove

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8

ionization enery: across a period

energy increases - same energy level but more protons so Zeff is greater and the electron is harder to remove

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9

ionization energy: exceptions

Group 13, Group 16

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10

group 13 exception

removing the last valence electron is easier then it should be because the full "s" sub level acts as a mini shield

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11

group 16 exception

due to electron repulsion, the 4th "p" electron is easier to remove

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12

second ionization energy

the amount of energy needed to remove the second (third,fourth,etc) valence electron from an atom increases

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13

electronegativity

the attraction an element has for the electrons in a chemical bond

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14

chemical bond

two electrons that are linking two atoms together

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15

electronegativity: down a group

electronegativity decreases - the more energy levels, the greater the shielding effect = the lower attraction for electrons

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16

electronegativity: across a period

electronegativity increases - there are more protons, so the shields stay the same and the Zeff is greater causing more electrons to be attracted to the nucleus

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17

electron affinity

the energy that is lost when an atom gains an electron - forms an anion; any time an attraction/bond is formed, energy is released;any time an attraction/bond is broken energy is gained

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18

electron affinity: down a group

electron affinity decreases - the increase in electron shields decreases the atoms ability to attract electrons

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19

electron affinity: across a period

electron affinity increases - it gains protons but the number of energy levels remains the same (the Zeff increases), so there is a greater attraction for electrons

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20

electron affinity: exceptions

group 2,15,18

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21

group 2 exception

"s" sublevel is full, so when it gains an electron, you need to add to the "p" sub level which is further away from the nucleus

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22

group 15 exception

all "p" sublevels are half way full, so another electron will experience electron repulsion, decreasing the attraction

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23

group 18 exception

the valence shell is full so there's no room for another electron

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